Chemistry Atomic Structure Quiz
No two electrons can have the same set of quantum numbers
Pauli's Exclusion Principle
All of the quantum numbers terms and definitions as well as other names: ___________________________________________________________________ n - Principle Energy Level- Main Energy Level - -> This can be found by either a given "n = ..." or a period on the periodic table ____________________________________________________________________ l - the weird l thing - Angular momentum - -> Different for each sublevel {s: l = 0} {p: l = 1} {d: l=2} {f: l = 3} ___________________________________________________________________ ml - not (milliliter) - still the weird l thing but now attached to the m - Magnetic orientation - -> Goes from the negative of the number to the positive and includes 0. Use this: {s: l = 0} {p: l = 1} {d: l=2} {f: l = 3} - So it will be: {-1, 0, 1} for p or {-2, -1, 0, 1, 2} for - - Found by using the sublevel of the electron ____________________________________________________________________ ms - m but now with an s - Magnetic Spin - -> This is the orientation of the electron (up or down arrow) - If it is an up arrow: + 1/2 - If it is a down arrow: - 1/2 - MUST have the (+) and (-) ____________________________________________________________________
Quantum Numbers
True or False: The principal quantum number designates the principal energy level occupied by the electron.
True
True or False: The s orbital has a spherical shape.
True
True or False: The threshold frequency is the minimum frequency of light that will eject electrons from a surface.
True
True or False: The wave lengths of infrared light are longer than those of visible light.
True
True or False: Two electrons in the same orbital cannot have the same spin quantum number.
True
A discrete bundle of electromagnetic energy: a) Photon b) Quantum c) Boson d) Lepton
a
A low-frequency wave has a _____ wavelength: a) long b) short c) variable d) high
a
A region of high probability of finding an electron: a) Atomic orbital b) Ground state c) Quantum d) Photon
a
According to the Aufbau principle, the _____ electrons are next in line of filling after the 6s electrons: a) 5d b) 4f c) 4d d) 6p
a
An increase in the quantum number n means _____ in the distance of the electron from the nucleus: a) an increase b) no change c) a decrease d) a variable response
a
Distance between two wave crests: a) Wavelength b) Frequency c) A really long way d) Orbital
a
Heisenberg Uncertainty Principle says, if the POSITION of n electron is known, what is unknown: a) Velocity b) Intensity c) Density d) Mass
a
Lowest energy level of an electron: a) Ground state b) Aufbau c) Wavelength d) Orbital
a
Separation of light into its different wavelengths: a) Spectrum b) Refraction c) Interference d) Diffusion
a
States that you can't know both the velocity and position of an electron simultaneously: a) Heisenberg Uncertainty Principle b) Hund's rule c) Aufbau Principle d) Pauli Exclusion Principle
a
The electron configuration for 12 Mg is: a)[Ne]3s² b)[Rn]3s² c)[Ne]3s²3p² d)[Rn]3s¹
a
The photoelectric effect was first demonstrated by: a) Albert Einstein b) Robot Millikan c) John Dalton d) J.J. Thomson
a
The spin quantum number has _____ values: a) two b) three c) one d) four
a
How can you determine the number of sublevels within an energy level: a) Count them off the periodic table b) n ^2 c) n d) 2(n ^2)
a and c
According to the Heisenberg Uncertainty Principle, the velocity and position of which of the following can never be measured very accurately? a) a traveling missile b) an electron in motion c) a hockey puck shot at the goal d) atomic emission lines
b
An atom's electron configuration describes: a) the shape of the electrons b) the arrangement of electrons c) the shape of electrons d) the shape of the orbitals
b
Arrangement of electrons around an atomic nucleus: a) Principle energy levels b) Electron configuration c) Sublevels d) Orbitals
b
Chromium has the following electron distribution: [Ar] 3d⁵ 4s¹. How many valence electrons does chromium have? a) six b) one c) five d) two
b
Each electron can be described by_____ quantum numbers: a) two b) four c) six d) eight
b
Energy needed to move an electron from one energy level to another: a) frequency b) quantum c) Wavelength d) Photon
b
How does the energy of an electron change if it moves farther from the nucleus: a) Increases then decreases b) Increases c) Decreases d) Stays the same
b
Lower orbitals are filled before upper orbitals is a statement of the: a) Hund's rule b) Aufbau principle c) Pauli exclusion principle d) de Broglie principle
b
One of the following statements about the photoelectric effect is not true: a) the idea was developed by Albert Einstein b) the effect can be seen at all frequencies of light c) light can behave as a particle d) electrons can be displaced when light shines on a metal surface
b
Orbitals can only have maximum of _____ electrons: a) 10 b) 2 c) 32 d) 8
b
Rule states that every orbital in a sublevel gets an electron before they pair up: a) Heisenberg Uncertainty Principle b) Hund's rule c) Aufbau Principle d) Pauli Exclusion Principle
b
The amplitude of a wave is its: a) frequency b) height c) wavelength d) velocity
b
The first five electron sublevels in order of filling are: a) 1s, 2s, 3s, 2p, 3p b) 1s, 2s, 2p, 3s, 3p c) 1s, 2s, 3s, 3p, 2s d) 1s, 3s, 2s, 3p, 2p
b
The units of velocity in the de Broglie wave equation are: a) km/sec b) m/sec c) cm/sec d) m/minute
b
Wavelength is defined as: a) the height of the wave b) the distance between two peaks c) the frequency of the wave d) the speed of the wave
b
What does the principal quantum number ( n ) indicate about an electron: a) Velocity b) Energy level c) orbital shape d) mass
b
What is the relationship between Energy and frequency of EM radiation: a) Inversely proportional b) Directly proportional c) They're warming up to each other d) Going to prom
b
What is the relationship between wavelength and frequency: a) Icy b) Inversely proportional c) Directly proportional d) They broke up
b
What is the speed of light: a) speed you travel to the parking lot after 7th period b) 3.0 x 10^8 m/s c) 5280 ft/s d) faster than greased lightning
b
Which of the following has the highest frequency: a) Infrared b) Ultraviolet c) Visible light d) Microwave
b
Who developed the modern Quantum Mechanical model? (Not Bohr!) a) Ernest Rutherford b) Erwin Schrodinger c) Neils Bohr d) Isaac Newton
b
How can you determine the number of electrons in an energy level: a) n ^2 b) 2(n ^2) c) Count the number of elements in that energy level d) n
b and c
All frequencies of light emitted by an element: a) Quantum b) Alphas c) Atomic Emission Spectrum d) Photon
c
An electron cloud: a) shows exactly where the electron is located b) gives a 75% probability of where the electron is located c) gives a 90% probability of where the electron is located d) gives a 65% probability of where the electron is located
c
Electron configuration superscripts indicate: a) orbital shape b) valence electrons c) number of electrons in a given sublevel d) number of reactive electrons
c
Frequency is represent by the Greek letter: a)μ b)σ c)ν d)λ
c
Number of wave cycles passing a point per second: a) Quantum b) Planck c) Frequency d) Wavelength
c
The highest allowable sublevel for n=3 is: a) s b) f c) d d) p
c
The spin quantum number gives: a) the angular momentum of the electron b) the rate of rotation of the electron c) the direction of spin of the electron d) the position of the orbital
c
The study of motion in large objects is called: a) traditional mechanics b) quantum mechanics c) classical mechanics d) quantized mechanics
c
The total number of allowable orbitals in the principle energy level n=3 is: a) 6 b) 12 c) 9 d) 3
c
The units of frequency are: a) meters/second b) cycles/meter c) cycles/second d) meters/minute
c
Valence electrons are: a) unpaired electrons in the outermost principle energy level b) all electrons in the outermost orbital c) electrons in the outermost principle energy level d) electrons with paired spin in the outermost principle energy level
c
Where are the exceptions to the electron configurations found in the d-sublevel? (borrow from "s") a) d^2, d^8 b) d^5, d^10 c) d^4, d^9 d) d^3, d^7
c
Which of these is NOT part of the Bohr atom model: a) Electrons orbit nucleus b) Nucleus made of protons c) Electron clouds d) Energy levels
c
How can you determine the number of orbitals within an energy level: a) n b) 2(n ^2) c) n ^2 d) Divide the # of electrons in that level by 2
c and d
A _____ is the minimum amount of energy that can be gained or lost by an electron: a) qualim b) quanta c) quentum d) quantum
d
If the principle quantum number n=4, the angular quantum number can have values for zero to: a) 2 b) 4 c) 1 d) 3
d
Tendency of electrons to enter orbitals of lowest energy first: a) Heisenberg Uncertainty Principle b) Pauli Exclusion Principle c) Hund's rule d) Aufbau Principle
d
The iodine atom has the electronic configuration [Kr] (4d^10) (5s^2) (5p^5). The number of valence electrons in this atom is: a) ten b) fifteen c) five d) seven
d
Wavelength is designated by the symbol: a)ν b)δ c)μ d)λ
d
What does ROY G BIV mean: a) Really Old Young Guys Being Incredibly Vile b) Rap On Your Growing Base In Vermont c) Row On You Good Boat In Venice d) Red, Orange, Yellow, Green, Blue, Indigo, Violet
d
What does the Pauli exclusion principle states that: a) all electrons have four quantum numbers b) quantum numbers are excluded for some elements c) two electrons in an element may have identical quantum numbers d) no two electrons in an element can have the same four quantum numbers
d
Which has the longest wavelength: a) Ultraviolet b) Microwave c) Gamma d) Radio
d
Which of the following doesn't describe the sublevel orbital cloud shapes: a) s - sphere b) d - four leaf clover c) p - dumbbell or propeller d) p - oval
d
Which of the following forms of electromagnetic radiation is most energetic: a) Ultraviolet b) Infrared c) Radio d) X - rays
d
Energy levels of electrons in an atom are...
discrete
1/s is also known as Hertz (Hz) and can also be written as inverse of second (sec ^-1) but they all mean the same thing and represent frequency
thing to remember
Be careful wth exponents when doing the math
thing to remember
Don't forget the (+) or (-) on the spin quantum numbers
thing to remember
If solving the question with 4 parts that involves the math remember these tips: 1) You're answer should not have a negative - if so, you did something wrong 2) It is final ( - ) initial, no multiplication and not the other way around 3) Don't forget to square the above mentioned numbers or forget that they are fractions 4) When finished, don't forget to use the inverse button on the calculator to get the real/correct answer and include measurements
thing to remember
The shapes of the orbitals are as follows: s - sphere p - dumbbell shape/ propeller shape d - four leaf clover f - (idk - its too complicated)
thing to remember
Things to know about electron configuration: 1) Valence electrons are outermost meaning s and p. D does not count and neither does f. 2) There can only be 8 valence electrons, no more. 3) The order is: Main Energy Level> Sublevel> Orbital> Electron 4) Only 2 electrons max in an orbital 5)Core electrons always equal the noble gas before the atom being used and only valence electrons matter - and d but not really. Refer to tip 1.
thing to remember
When a question asks: "what number of orbitals are in energy level 4 or n=4" you must include d and/or f if it applies. You can solve this type o question by counting the number of elements in each row and then dividing by two, but it is crucial to remember the above mentioned tip when doing it or else it will be wrong.
thing to remember
Higher energy levels will be filled before lower energy levels - all the "arrows" will face up if there is only 1 arrow in the box - again, this is referring to the boxes and arrows in the electron configuration diagrams
Aufbau Principle
True or False: An electron and a photon are of equal mass.
False
True or False: Classical physics could completely explain the photoelectric effect.
False
True or False: The Bohr model of the atom explains the emission lines of iron.
False
Location and velocity of an electron cannot be known simultaneously - if you know one, you will not know the other - Hint: Think of the west boca road story. If you are moving, your exact location cannot be mapped but the velocity at which you are moving can. And if you are standing still, the exact point at which you are at can be recorded but not your velocity.
Heisenberg Uncertainty Principle
Before any of the squares are doubled up, all of the squares have to be filled - this refers to electron configuration diagram squares and the arrows
Hunds Rule
The Visible Spectrum of light spans the range of approximately...
400-700 nm
